The total pressure of the mixture of gases is equal to the sum of the pressure of each gas as if it is alone in the container. The partial pressure of a component of the mixture is said to be equal to the product of the total pressure and the mole fraction of the component in the mixture.
Partial pressure of hydrogen gas = 1.24 atm x .25 = 0.31 atm
Partial pressure of the remaining = 1.24 atm x (1-.25) = 0.93 atm
Answer:
2.34 molality
Explanation:
Mole weight of KOH ( using periodic table ...rounded to 3 s.f.) =
56.1 gm/mole
Number of moles in 43.2 g
43.2 g / 56.1 gm / mole =.770 mole
molality = .770 mole / .329 kg = 2.34 m
Answer:
-1151.5 J
Explanation:
Given that:
The supplies energy = 245 L
The energy used in the expansion of gas = Pressure ×ΔV (change in volume)
At standard conditions;
Pressure = 105 × 10³ Pa
energy used in the expansion = 105 × 10³ Pa × (38.6 - 25.3)L
= 1396.5 J
Thus, the change in the energy of gas = 245 - 1396.5 J
= -1151.5 J
Hence, we can conclude that the gas has lost its own energy in the process of expansion.
The answer is: both choices a and b.
The base SI unit for molar mass is kg/mol, but chemist more use g/mol (gram per mole).
For example, the molar mass of fluorine is 38.00 g/mol.
M(F₂) = 2 · Ar(F) · g/mol.
M(F₂) = 2 · 19.00 · g/mol.
M(F₂) = 38.00 g/mol.
Molar mass M represent the mass of a substance (in this example molecule of florine) divided by the amount of substance.
Ar is the atomic weight of a chemical element (in this example fluorine).
A buffer is a solution of weak acid and conjugate base or weak base and conjugate acid used to resist pH change with added solute. <span />
